Balancing Redox Reaction by Ion Electron Method (Half Reaction Method)

Balancing the e- charge and making the electron gain or lose in the half racing is very important to “balance the following redox reaction by ion electron method.” In a chemical reaction, assign the numbers of oxidation d=for every atom, and the proper identification of redox couples in the chemical reaction is very important for balancing the redox reaction of the electric particles. In order to balance atoms in every half-reaction, it is essential for balancing H and O atoms, adding H2O atoms along with hydrogen atoms with two sides is very important for balancing the redox reaction in a chemical equation.    

“Balance the following redox reaction” by the ion-electron method: Examples

A balanced redox reaction is the simplest manner which can be balanced by utilising some important procedures:

• The equation is dissected into two half-reactions.
• Each half-reaction for charge and mass is balanced.
• The transfiguration of the number of electrons is equalised in every half-reaction.
• The half-reaction is then added collaboratively.

 Among all the redox, one instance is considered to “balance the following redox reaction by ion electron method”:

• MNO4– (aq) + I– (aq) → MnO2(s) + I2 (s) in basic medium

Stage 1

“Half-reaction” by oxidation: “l (aq) → l2(s)”

“Half-reaction” by reduction: “Mn O–4(aq)  → MnO2(aq)”

Stage 2

Getting balanced in the half reaction by oxidation

“2l–(aq) → l2(s)”

For balancing the charge 2 e– is added to RHS

“2l–(aq) → l2(s) + 2e-”

Stage 3

Addition of 3 electrons to LHS and 4 OH– to the RHS of the reaction respectively

“MnO–4(aq) + 3e–  →MnO2 (aq)”

“MnO–4(aq) + 3e–  →MnO2 (aq) + 4OH–”

Stage 4

Addition of two water molecules

“MnO–4(aq) + 2H2O + 3e–  →MnO2 (aq) + 4OH–”

Stage 5

Equalising electrons numbers

“6l–(aq) → 3l2(s) + 2e–”

“2MnO–4(aq) + 4H2O + 6e–  → 2MnO2(s) + 8OH–(aq)”

Stage 6

Addition of two half-reactions to get balanced redox reaction

“6l–(aq) +  2MnO–4(aq) + 4H2O (l) →  3l2(s) + 2MnO2(s) + 8OH–(aq)”

Ion electron method: Concept

“Ion electron method” is also termed as a half-reaction method where the “redox equation” is discredited into two half equations. The two half equation is mentioned to be “one for oxidation” and “one for reduction”. Among these two equations, every equation is balanced distinctly and then merged to provide a balanced redox equation. Ions are generally created by summing of electrons or the deduction of electrons from neutral molecules or atoms or another ion by an amalgamation of ions with different particles. “Ion electron method” differs from the oxidation number method which gets balanced depending on ionic charges in the oxidation number of reductants and oxidants. The “ion-electron method” permits singles to balance the reactions of redox irrespective of their complexity. The method is described in two examples where I– gets highly oxidised to “IO3-” by “MNO4-” which then deduces to “Mn2+”. The ions impact the configuration of electrons when a single atom loses or gains electrons, it becomes an ion. 

State balance by half-reaction method

“The balance by half-reaction method” demonstrates the manner to balance the redox reaction. It implies a dissection of the overall down of equation into the part of reduction and oxidation. The “half-reaction method” reflects the electron’s movement within the reduction or oxidation stage of the reaction. The “balance by half-reaction method” in redox reaction in mainly two ways:

• They are utilized to illustrate the occurrence of reactions in the cell of electrochemicals. Every “half-reaction” presents the reaction happening between two electrodes.
• They can be utilized in balancing “redox reaction” in the acidic or basic reaction conditions such as OH–, H2O or H+ are added to stabilize the reaction.

Conclusion 

Two different methods are principally used to make “balance the following redox reaction by ion electron method” is “oxidation number method” as well as the “half-reaction method”. The use of the accurate formula for electrical products as well as reactions of the chemical reaction determines the oxidation process. The ion-electron method in the chemical equation allows the balancing of the redox reaction as per the material complexity. The oxidation method of electric particles guides to determine if the number of oxidation of each atom and making electron loss or grain changes the whole number of rest atoms. “Mg ( s ) → M g 2 + ( aq ) + 2 e” is an equation of ion-electron and in that equation, the number of reduction is just the opposite of the oxidation process.